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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question
![**Chemical Equilibrium Problem:**
**Reaction:**
\[ 1 \, \text{A} + 1 \, \text{B} \rightleftharpoons 3 \, \text{C} \]
**Given:**
- The initial concentration of \([\text{A}]\) is 1.20 M.
- The initial concentration of \([\text{B}]\) is 1.50 M.
- The equilibrium constant (\(K_c\)) is 0.0000076.
**Problem:**
What is the concentration of \([\text{C}]\) at equilibrium?
**Note:** You may assume the 5% rule is valid for this calculation.
In solving this problem, utilize the equilibrium expression derived from the balanced chemical equation and apply the 5% rule to simplify your calculations if applicable.](https://content.bartleby.com/qna-images/question/f4909d4a-b929-4db1-b816-76d439c1817d/877d31f9-0958-4e87-b01d-64a124b2ca20/du1876_thumbnail.jpeg)
Transcribed Image Text:**Chemical Equilibrium Problem:**
**Reaction:**
\[ 1 \, \text{A} + 1 \, \text{B} \rightleftharpoons 3 \, \text{C} \]
**Given:**
- The initial concentration of \([\text{A}]\) is 1.20 M.
- The initial concentration of \([\text{B}]\) is 1.50 M.
- The equilibrium constant (\(K_c\)) is 0.0000076.
**Problem:**
What is the concentration of \([\text{C}]\) at equilibrium?
**Note:** You may assume the 5% rule is valid for this calculation.
In solving this problem, utilize the equilibrium expression derived from the balanced chemical equation and apply the 5% rule to simplify your calculations if applicable.
Expert Solution
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Step 1
While calculating the concentrations of the individual components in an equilibrium, the amount of reactant dissociated, say ‘x’ by a time, ‘t’, then the subtracting x from the value of initial concentration is not necessary if, x is less than or equal to 5%.
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
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- Consider the reaction A + B C+D, which has an equilibrium constant, K, equal to 3.4 x 102. If one begins a reaction by placing 0.600 moles of A in a 1.0 L container as well as 0.150 moles of 1. B, what will be the equilibrium concentrations of A, B, C, and D? Write your answers in the spaces provided below. a. [А] b. [B]= [C]= С. d. [D]= Once the reaction in problem 1 reaches equilibrium, some additional B is injected into the flask 2. from an outside source. LeChatelier's principle says the reaction will (circle one): be unchanged shift to the right shift to the left Pyridine is a weak base with a Kb 1.7 x 109. If 0.300 moles of pyridine is added to 1.00 L of 3. water, what will be the equilibrium concentrations of the species below: a. [Pyridine] = b. [Pyridine-H] (the pyridinium ion) [ОН-] 3 С. What is the pH of the solution in problem 4 (above)? .arrow_forwardConsider the reaction. PCI, (g) = PCI, (g) + Cl,(g) Ke = 0.0420 The concentrations of the products at equilibrium are [PC13] = 0.100 M and [Cl2] = 0.260 M. What is the concentration of the reactant, PCI5, at equilibrium? [PCI5] = Marrow_forwardNitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2 HNO3(aq)+NO(9)→3 NO2(g)+H,0(1) At a certain temperature, a chemist finds that a 4.0 L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount HNO3 5.2 g NO 19.8 g NO, 7.9 g H,O 134.3 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. °C K_ = 0 x10 Carrow_forward
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